................[HgCl2]M............ [C2O4-2]M........ Rate(M/sec)
1..................0.105....................0.15...............1.8 x 10-5
2 .................0.105....................0.30...............7.2 x 10-5
3...................0.052...................0.30...............3.5 x 10-5
4..................0.052....................0.15...............8.9 x 10-6
5 .................0.200....................0.45.....................X
6..................0.35..........................y.................5.0 x 10-5

a) Determine the rate law
b) Calculate k
c) Determine the values for X and Y
3. Butadiene, C4H6, dimerizes to C8H12 with a 1st order rate constant of 0.014 L/mol sec. Starting with 0.025 M
a) What will be the concentration after 3.00 minutes?
b) How long will it take the concentration to drop to 0.0065 M?

Solution Preview

1.
6PCl5 -> 6PCl3+6Cl2 (-6*(III))
10PCl3+5O2 -> 10Cl3PO (10*(IV))
P4O10 -> P4+5O2 (-(II)).
(I)-6*(III)+10*(IV)-(II): we could obtain our reaction.
Delta H = -1225.6-6*(-84.2)+10*(-285.7)-(-2967.3)= -610.1 kJ

2.
a)
When [C2O4-2] ...

Solution Summary

The expert calculates deltaH for a reaction using kinetic rate laws.

The following data were acquired in an iodination experiment involving acetone.
Trial Volume of 0.0010
( )
Volume of 0.050
( )
Volume of 1.0 acetone
( )
Volume of water
( )
Temperature
( )
Reaction time
( )
A 5.0 10.0 10.0 25.0 25.0 130
B 10.0 10.0 10.0 20.0 25.0 249
C 10.0 20.0 10.0 10.0 25.0 128
D 10.0

Consider the reaction of peroxydisulfate ion S2O8 ^2 - with iodide ion (I-) in aqueous solution:
S2O8^2-(aq) + 3I-(aq) 2SO4 ^2-(aq) + I3-(aq)
At a particular temperature the initial rate of disappearance of S2O8^2- varies with reactant concentrations in the following manner:
Experiment [S2O8 2-] (M) [I-] (M) Initial Rat

Problem.
The kinetics of an aqueous phase decomposition of A is investigated in two CSTR's in series, the first having half the volume of the second. At steady state with a feed concentration of 4 gmol/lit., and mean residence time of 65 sec in the second reactor, the concentration of feed to second from the first is found to b

The 1st order composition of hydrogen peroxide has a rate constant of 7.30 X 10-4 s^-1 at 25 degrees C. Determine the percent of hydrogen peroxide that has decomposed after the first 500 seconds?
Since I do not have the initial concentration, I was going to use the half life equation and take the percentage of that. The miss

1) Explain the concept of chemical kinetics and the various factors that influence reaction states.
2) Relate experimental measurements to reaction rates and the ratelaws.
3) Determine the order of reaction, the ratelaw, the rate constant, and the rate of concentrations.
4) Solve first-order rate problems.

Using this data calculate the rate law for the reaction A + B -> C
[A] (M) [B] (M) Initial rate (M/s)
0.10 0.10 0.0092
0.20 0.20 0.0184
0.20 0.40 0.0368

The reaction A produces B + C is known to be zero order in A and to have a rate constant of 5.0 x 10 superscript-2 mol/L x sec. @ 25 degrees C. An experiment was run at 25 degrees C where [A]0 = 1.0 x 10 superscript-3 M.
a) Write the integrated law for this reaction
b) Calculate the half-life for this reaction
c) Calculate

Consider the following reaction:
A+B----AB
For a certain set of initial concentrations of A and B, it takes 10 seconds to produce 0.1 mmol of AB at 20 degrees celsius and 150 seconds at 0 degrees celsius. What is the ratio of the rate at 20 degrees to that at 0 degrees?

In aqueous solution, the reaction of A to form B has the following rate expression:
-d[A]/dt = k[A]{1 + k'[H+]}
From the pH dependence of the reaction, k' was found to be 1.0 x 10e5 M-1. In a pH 4.0 buffer, it took 5 min for a 0.30 M solution of A to react to give 0.15 M solution B. Calculate the value of k and g

For the reaction given below, the frequency factor A is 8.7 x 10^12 s-1 and the activation energy is 63 kJ/mol.
NO(g) + O3(g) ----> NO2(g) + O2(g)
What is the rate constant for the reaction at 70°C?